9KClO + 2H3PO4 → 3KClO2 + 2K3PO4 + 3Cl2↑ + 3H2O
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- Reaction of potassium hypochlorite and phosphoric acid
The reaction of potassium hypochlorite and phosphoric acid yields potassium chlorite, potassium phosphate, , and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium hypochlorite and phosphoric acid
General equation
- Reaction of self redoxing species and acid
- Self-redoxing speciesSelf redox agent + AcidNon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium hypochlorite and phosphoric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO | Potassium hypochlorite | 9 | – | Self redoxing |
| H3PO4 | Phosphoric acid | 2 | – | Acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KClO2 | Potassium chlorite | 3 | Oxidized | – |
| K3PO4 | Potassium phosphate | 2 | – | – |
| 3 | Reduced | – | ||
| H2O | Water | 3 | – | – |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium hypochlorite and phosphoric acid◆
ΔrG −82.0 kJ/mol K 2.32 × 1014 pK −14.37
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −72.0 | −82.0 | 34 | – |
per 1 mol of | −8.00 | −9.11 | 3.8 | – |
per 1 mol of | −36.0 | −41.0 | 17 | – |
per 1 mol of | −24.0 | −27.3 | 11 | – |
per 1 mol of | −36.0 | −41.0 | 17 | – |
| −24.0 | −27.3 | 11 | – | |
per 1 mol of | −24.0 | −27.3 | 11 | – |
Changes in aqueous solution (2)
- Reaction of potassium hypochlorite and phosphoric acid◆
ΔrG −61.2 kJ/mol K 5.27 × 1010 pK −10.72
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −142.2 | −61.2 | −272 | – |
per 1 mol of | −15.80 | −6.80 | −30.2 | – |
per 1 mol of | −71.10 | −30.6 | −136 | – |
per 1 mol of | −47.40 | −20.4 | −90.7 | – |
per 1 mol of | −71.10 | −30.6 | −136 | – |
| −47.40 | −20.4 | −90.7 | – | |
per 1 mol of | −47.40 | −20.4 | −90.7 | – |
Changes in aqueous solution (3)
- Reaction of potassium hypochlorite and phosphoric acid◆
ΔrG −329.7 kJ/mol K 5.77 × 1057 pK −57.76
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −93.9 | −329.7 | 791 | – |
per 1 mol of | −10.4 | −36.63 | 87.9 | – |
per 1 mol of | −47.0 | −164.8 | 396 | – |
per 1 mol of | −31.3 | −109.9 | 264 | – |
per 1 mol of | −47.0 | −164.8 | 396 | – |
| −31.3 | −109.9 | 264 | – | |
per 1 mol of | −31.3 | −109.9 | 264 | – |
Changes in aqueous solution (4)
- Reaction of potassium hypochlorite and phosphoric acid◆
ΔrG −308.9 kJ/mol K 1.31 × 1054 pK −54.12
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −164.1 | −308.9 | 485 | – |
per 1 mol of | −18.23 | −34.32 | 53.9 | – |
per 1 mol of | −82.05 | −154.4 | 243 | – |
per 1 mol of | −54.70 | −103.0 | 162 | – |
per 1 mol of | −82.05 | −154.4 | 243 | – |
| −54.70 | −103.0 | 162 | – | |
per 1 mol of | −54.70 | −103.0 | 162 | – |
Changes in aqueous solution (5)
- Reaction of potassium hypochlorite and phosphoric acid◆
ΔrG −82.0 kJ/mol K 2.32 × 1014 pK −14.37
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −72.0 | −82.0 | 34 | – |
per 1 mol of | −8.00 | −9.11 | 3.8 | – |
per 1 mol of | −36.0 | −41.0 | 17 | – |
per 1 mol of | −24.0 | −27.3 | 11 | – |
per 1 mol of | −36.0 | −41.0 | 17 | – |
| −24.0 | −27.3 | 11 | – | |
per 1 mol of | −24.0 | −27.3 | 11 | – |
Changes in aqueous solution (6)
- Reaction of potassium hypochlorite and phosphoric acid◆
ΔrG −61.2 kJ/mol K 5.27 × 1010 pK −10.72
| Standard enthalpy of reaction ΔrH° kJ · mol−1 | Standard Gibbs energy of reaction ΔrG° kJ · mol−1 | Standard entropy of reaction ΔrS° J · K−1 · mol−1 | Standard heat capacity of reaction at constant pressure ΔrCp° J · K−1 · mol−1 | |
|---|---|---|---|---|
per 1 mol of Equation | −142.2 | −61.2 | −272 | – |
per 1 mol of | −15.80 | −6.80 | −30.2 | – |
per 1 mol of | −71.10 | −30.6 | −136 | – |
per 1 mol of | −47.40 | −20.4 | −90.7 | – |
per 1 mol of | −71.10 | −30.6 | −136 | – |
| −47.40 | −20.4 | −90.7 | – | |
per 1 mol of | −47.40 | −20.4 | −90.7 | – |
Thermodynamic data of reactants
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| KClO (ai) | -359.4[1] | -320.0[1] | 146[1] | – |
| H3PO4 (cr) | -1279.0[1] | -1119.1[1] | 110.50[1] | 106.06[1] |
| H3PO4 (l) | -1266.9[1] | – | – | – |
| H3PO4 (ai) | -1277.4[1] | -1018.7[1] | -220.3[1] | – |
| H3PO4 (ao) | -1288.34[1] | -1142.54[1] | 158.2[1] | – |
| H3PO4 (cr) 0.5 hydrate | -1431.3[1] | -1242.1[1] | 129.16[1] | 126.02[1] |
| H3PO4 (cr) 1 hydrate | -1568.83[1] | – | – | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (l):Liquid, (ao):Un-ionized aqueous solution
Thermodynamic data of products
| Chemical formula | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
|---|---|---|---|---|
| KClO2 (ai) | -318.8[1] | -266.1[1] | 203.8[1] | – |
| K3PO4 (cr) | -1950.2[1] | – | – | – |
| K3PO4 (ai) | -2034.7[1] | -1868.7[1] | 87.2[1] | – |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[1] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
| H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -359.4 kJ · mol−1
- ^ ΔfG°, -320.0 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1
- ^ ΔfH°, -1279.0 kJ · mol−1
- ^ ΔfG°, -1119.1 kJ · mol−1
- ^ S°, 110.50 J · K−1 · mol−1
- ^ Cp°, 106.06 J · K−1 · mol−1
- ^ ΔfH°, -1266.9 kJ · mol−1
- ^ ΔfH°, -1277.4 kJ · mol−1
- ^ ΔfG°, -1018.7 kJ · mol−1
- ^ S°, -220.3 J · K−1 · mol−1
- ^ ΔfH°, -1288.34 kJ · mol−1
- ^ ΔfG°, -1142.54 kJ · mol−1
- ^ S°, 158.2 J · K−1 · mol−1
- ^ ΔfH°, -1431.3 kJ · mol−1
- ^ ΔfG°, -1242.1 kJ · mol−1
- ^ S°, 129.16 J · K−1 · mol−1
- ^ Cp°, 126.02 J · K−1 · mol−1
- ^ ΔfH°, -1568.83 kJ · mol−1
- ^ ΔfH°, -318.8 kJ · mol−1
- ^ ΔfG°, -266.1 kJ · mol−1
- ^ S°, 203.8 J · K−1 · mol−1
- ^ ΔfH°, -1950.2 kJ · mol−1
- ^ ΔfH°, -2034.7 kJ · mol−1
- ^ ΔfG°, -1868.7 kJ · mol−1
- ^ S°, 87.2 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1